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This document explores the fundamental concepts of states of matter, phase changes, and the energy associated with these transitions. It includes calculations for boiling ice and details on heating curves for water, discussing specific heat capacities and enthalpy changes. Additionally, it examines vapor pressure vs. temperature, the impact of intermolecular hydrogen bonds, and the dissolution of ionic compounds in water. The document further addresses the properties of crystalline solids, including various lattice types and their interactions, providing insights into material behavior under different conditions.
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Liquids & Solids Dr. Ron Rusay Fall 2001
Heating Curve for H2O Cpvap=0.48 cal/g xoC Hvapor= +540 cal/g Cpliq=1.00 cal/g xoC Hfusion= +80.0 cal/g Cpice=0.50 cal/g xoC Calculate the heat necessary to completely boil 1.0 kg of ice that is at -5oC. +722.5 kcal = +3,023 kJ
Periodicity: Boiling Point Boiling Point: Temperature at which the vapor pressure of the liquid equals the atmospheric pressure. Higher vapor pressure : Lower boiling point. Does water boil at the same temperature in Concord and Tahoe?
Boiling Points of Simple Hydrogen Compounds What can explain the trends?
Intermolecular Hydrogen Bonds in H2O Besides oxygen, both nitrogen and fluorine form intermolecular hydrogen bonds. Other atoms DO NOT.
Views of Water 104.5o Angle Dipole Moment
Intermolecular ForcesIonic & Polar Interactions:+ and - ; + ---- -
FG11_004.JPG Dipole-Dipole Forces
Surface Forces of a Liquid Viscosity & Surface Tension of liquids are directly related to the strength of the intermolecular forces: Eg. Water versus gasoline. 1.00 vs 0.20 centipoise and 70 vs. 15 dynes/cm 2 respectively.
Three Types of Crystalline Solids Ionic Molecular Metallic
